Pb(NO3)2 + 2KI ==> PbI2 + 2KNO3
Convert 1.23 mg Pb(NO3)2 to moles. moles = grams/molar mass
Using the coefficients in the balanced equation, convert moles Pb(NO3)2 to moles KNO3.
Now convert moles KNO3 to grams. g = moles x molar mass.
Convert 1.23 mg Pb(NO3)2 to moles. moles = grams/molar mass
Using the coefficients in the balanced equation, convert moles Pb(NO3)2 to moles KNO3.
Now convert moles KNO3 to grams. g = moles x molar mass.
The balanced equation for the reaction is as follows:
Pb(NO3)2 + 2 KI -> PbI2 + 2 KNO3
From the equation, we can see that each mole of lead(II) nitrate reacts with 2 moles of potassium iodide to produce 1 mole of lead(II) iodide and 2 moles of potassium nitrate.
1. Convert the mass of lead nitrate consumed to moles using its molar mass.
The molar mass of Pb(NO3)2 can be calculated as follows:
Pb: atomic mass = 207.2 g/mol
N: atomic mass = 14.0 g/mol
O: atomic mass = 16.0 g/mol
Total molar mass of Pb(NO3)2 = (207.2 g/mol) + 2 * (14.0 g/mol + 3 * 16.0 g/mol) = 331.2 g/mol
Now, calculate the number of moles of Pb(NO3)2:
moles = mass / molar mass = 1.23 mg / 331.2 g/mol
2. Determine the moles of potassium nitrate produced.
Since the stoichiometry of the balanced equation indicates that 1 mole of lead(II) nitrate produces 2 moles of potassium nitrate, the moles of potassium nitrate will be twice the moles of lead(II) nitrate.
moles of KNO3 produced = 2 * moles of Pb(NO3)2
3. Convert the moles of potassium nitrate produced to mass using its molar mass.
The molar mass of KNO3 can be calculated as follows:
K: atomic mass = 39.1 g/mol
N: atomic mass = 14.0 g/mol
O: atomic mass = 16.0 g/mol
Total molar mass of KNO3 = 39.1 g/mol + 14.0 g/mol + 3 * 16.0 g/mol = 101.1 g/mol
Now, calculate the mass of KNO3 produced:
mass = moles * molar mass
By following these steps, you can calculate the mass of potassium nitrate produced when 1.23 mg of lead nitrate reacts.